properties of solutions lesson 2. measuring concentration concentration = amount of solute/amount...
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Properties of SolutionsProperties of Solutions
Lesson 2Lesson 2
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Measuring concentration Measuring concentration
Concentration = amount of solute/amount Concentration = amount of solute/amount of solutionof solution
Weight/volume percentWeight/volume percent Mass solute in g/volume of soln in mL x 100%Mass solute in g/volume of soln in mL x 100%
Weight/weight percentWeight/weight percent Mass solute in g/mass solution in g x 100%Mass solute in g/mass solution in g x 100%
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–3
Molarity = Moles of solute/Liters of Solution (M)
Molality = Moles of solute/Kg of Solvent (m)
Mole Fraction=Moles solute/total number of moles
Mass %=Mass solute/total mass x 100
Concentration
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–4
Molarity = Moles of solute/Liters of Solution (M)
Molality = Moles of solute/Kg of Solvent (m)
Mole Fraction=Moles solute/total number of moles
Mass %=Mass solute/total mass x 100
Concentration
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–5
Molarity = Moles of solute/Liters of Solution (M)
Molality = Moles of solute/Kg of Solvent (m)
Mole Fraction=Moles solute/total number of moles
Mass %=Mass solute/total mass x 100
Concentration
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Molarity
moles of soluteMolarity ( ) =
liters of solution M
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–7
A sample of NaNO3 weighing 8.5 grams is placed in a 500 ml volumetric flask and distilled water was added to the mark on the neck of the flask. Calculate the Molarity of the resulting solution.
Convert the given grams of solute to moles of solute :
Convert given ml of solution to liters
Apply the definition for Molarity: Molarity = moles NaNO3 / volume of the solution in liters
M = 0.1 mole / .500 liters = 0.200 Molar NaNO3
33
33
1 mole NaNO
858.5 g NaNO 0.1 mole
g N
NaNOaNO
1 liter
1000 ml500 ml 0.5 liter
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Exercise #1
You have 1.00 mol of sugar in 125.0 mL of solution. Calculate the concentration in units of molarity.
8.00 M
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Exercise #2
You have a 10.0 M sugar solution. What volume of this solution do you need to have 2.00 mol of sugar?
0.200 L
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Exercise #3
Consider separate solutions of NaOH and KCl made by dissolving 100.0 g of each solute in 250.0 mL of solution. Calculate the concentration of each solution in units of molarity.
10.0 M NaOH
5.37 M KCl
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–11
Molarity = Moles of solute/Liters of Solution (M)
Molality = Moles of solute/Kg of Solvent (m)
Mole Fraction=Moles solute/total number of moles
Mass %=Mass solute/total mass x 100
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Molality
moles of soluteMolality ( ) =
kilogram of solvent m
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Exercise #4
A solution of phosphoric acid was made by dissolving 8.00 g of H3PO4 in 100.0 mL of water. Calculate the molality of the solution. (Assume water has a density of 1.00 g/mL.)
0.816 m
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–14
Molarity = Moles of solute/Liters of Solution (M)
Molality = Moles of solute/Kg of Solvent (m)
Mole Fraction=Moles solute/total number of moles
Mass %=Mass solute/total mass x 100
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–15
Determine the mole fraction of KCl in 3000 grams of aqueous solution containing 37.3 grams of Potassium
Chloride KCl.
1. Convert grams KCl to moles KCl using the molecular weight of KCl
2. Determine the grams of pure solvent water from the given grams of solution and solute
Total grams = 3000 grams = Mass of solute + Mass of water Mass of pure solvent = (3000 - 37.3) gram
= 2962.7 gram
1 mole KCl
74.6 g K37.3 g KCl 0.5 mo
Clle KCl
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–16
Determine the mole fraction of KCl in 3000 grams of aqueous solution containing 37.3 grams of Potassium
Chloride KCl.
3. Convert grams of solvent H2O to mols
4. Apply the definition for mole fraction mole fraction = moles of KCl / Total mols of KCl and water =
0.5 / (0.5 + 164.6) = 0.5 / 165.1 = 0.00303
2
1 mol
18.0 grams2962.7 grams water 164.6 mols H O
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Mole Fraction
AA
molesMole fraction ( ) =
total moles of solution
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Exercise #5
A solution of phosphoric acid was made by dissolving 8.00 g of H3PO4 in 100.0 mL of water. Calculate the mole fraction of H3PO4.
(Assume water has a density of 1.00 g/mL.)
0.0145
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Mass Percent
mass of soluteMass (weight) percent = 100%
mass of solution
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Exercise #6
What is the percent-by-mass concentration of glucose in a solution made my dissolving 5.5 g of glucose in 78.2 g of water?
6.6%
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Copyright © Houghton Mifflin Company. All rights reserved. 17a–21
Assuming the density of water to be 1 g/mL we approximate the density of a dilute aqueous solution to be 1 g/mL
1 ppm = 1 μg/mL = 1 mg/L
1 ppb = 1 ng/mL = 1 μg/L
1 g1 ppm =
1 g
1 g 1 g
1
1 g
1 ml g 1 ml
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MolarityMolarity
Concentration is usually expressed in Concentration is usually expressed in terms of molarity:terms of molarity:
Moles of solute/liters of Moles of solute/liters of solutionsolution (M) (M)
Moles of solute = molarity x volume of solutionMoles of solute = molarity x volume of solution
Moles = M x VMoles = M x V
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Molarity and concentrationMolarity and concentration
Molarity:Molarity:
M = moles solute/liter of solutionM = moles solute/liter of solution DilutionDilution
MM11VV11 = M = M22VV22
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ExampleExample
What is molarity of 50 ml solution containing What is molarity of 50 ml solution containing 2.355 g H2.355 g H22SOSO44?? Molar mass HMolar mass H22SOSO44 = 98.1 g/mol = 98.1 g/mol
Moles HMoles H22SOSO44 = .0240 mol = .0240 mol (2.355 g/98.1 g/mol)(2.355 g/98.1 g/mol)
Volume of solution = 50 mL/1000 mL/L = .050 LVolume of solution = 50 mL/1000 mL/L = .050 L Concentration = moles/volumeConcentration = moles/volume
= .0240 mol/.050 L = 0.480 M= .0240 mol/.050 L = 0.480 M
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Solution stoichiometrySolution stoichiometry How much volume of one solution to react with another How much volume of one solution to react with another
solutionsolution Given volume of A with molarity MGiven volume of A with molarity MAA
Determine moles ADetermine moles A Determine moles BDetermine moles B Find target volume of B with molarity MFind target volume of B with molarity MBB
Volume Bmol = MV Mole:mole ratio V = mol/MVolume A Moles A Moles B